Unit 3 Ray Tedder s Chemistry I Test Prep Guide page 1
|
|
- Abner White
- 5 years ago
- Views:
Transcription
1 Unit 3 Ray Tedder s Chemistry I Test Prep Guide page 1 Bonding Unit 3: Chemistry I In this unit all students must be able to Understand that the structure of molecules is the result of nonmetals sharing electrons in order to form stable outer-energy-level configuration. This sharing of electrons creates what is called a covalent bond. One way to represent the sharing of electrons is by using the orbital notation system that you learned and used in the last unit. You can write the orbital notation for different elements and use those illustrations to show how the valence level orbitals overlap in covalent bonding. Examples: Hydrogen has 1 electron, with an orbital notation of: H: Oxygen has 8 electrons, with an orbital notation of: 2p Before oxygen can bond covalently, it must hybridize. In hybridization, the 2 kinds of valence level orbitals change into one kind of valence level orbital. The valence level is the highest primary electron energy level. This case, the highest primary energy level is 2. The hybridized electron configuration of oxygen looks like this: Unhybridized orbital notation for oxygen Unhybridized orbital notation for oxygen O: 2s O: O: 2s 2p 2 These unhybridized valence orbitals combine and form these 4 equal hybridized orbitals If 2 hydrogen atoms are combined with one oxygen atom, then each of the halffilled (single arrow) hydrogen electron orbitals are combined with each of the half-filled (single arrow) oxygen electron orbitals, creating a set of filled valence level orbitals: o Draw Lewis dot structures for simple molecules Lewis dot structures or Lewis dot formulas are drawings that show the arrangement of electrons in 2 dimensions. Molecules are formed when atoms bond together covalently, which means they bond in a way in which they share This illustration shows modified orbital notations for hydrogen and oxygen before they share electrons (arrows show where in the orbitals the electrons will be shared and will overlap). H: H: 2 O: This illustration shows a combine modified orbital notation for hydrogen and oxygen after they share electrons. Notice how the orbitals overlap. H 2 O: O: 2 Figure 3.1. The illustration above shows an orbital notation illustration of how sharing of electrons occur to form covalent bonds. :H :H
2 Unit 3 Ray Tedder s Chemistry I Test Prep Guide page 2 electrons. The sharing of electrons allows atoms to have enough electrons to fill their valence level. The valence level is the highest primary electron energy level of an atom. You can also think of the valence level of an atom as the outer-most primary energy level of an atoms electron cloud. Lewis dot structures, Lewis dot diagrams, Lewis dot formulas Lewis dot structures* show the shared pairs of electrons and also show the lone pairs (sometimes called unshared pairs) of electrons. A Lewis structure can be drawn for any covalently-bonded molecule, any polyatomic ion, and any coordination compound. We will only be learning about covalently-bonded molecules in this unit. Later, we will learn how Lewis dot structures can be also be used to illustrate ionic bonding. First, however, I will give you a method for creating these Lewis dot structures. *Note: These structures are also called formulas, diagrams, or drawings. Most of the time, atoms share electrons in a way that gives each atom 8 electrons in the valance level. Hydrogen (H) is an exception; it only wants to get 2 electrons (2 electrons will give hydrogen the noble gas electron configuration of helium). Remember that valence electrons are those in the highest primary level. You can figure out how many electrons there are in the highest primary level by drawing the orbital notation or writing the electron configurations. H: 1 H 1 or H or H or H:. Orbital notation for hydrogen Electron configuration for hydrogen Lewis dot formula for hydrogen (Note: It doesn t matter on which side you place the single electron) Hydrogen (symbol H) has only has 1 valence electron. This electron is represented by the one arrow in the orbital notation. This electron is also represented by the superscript 1 in the orbital notation. It is also represented by the single dot around the hydrogen symbol in the Lewis dot formula. O: 2s 2p Orbital notation for oxygen O: 2 2s 2 2p 4 Electron configuration for oxygen Definitions: A shared pair of electrons is a) any circled any pairs of electrons between atoms in a sharing arrangement, b) and electrons in between atoms in a Lewis dot formula, or c) any lines representing pairs of electrons in a Lewis structure or formula. A lone pair of electrons is any pair of electrons in the valence level that is NOT involved in bonding. In a Lewis dot formula, or Lewis structure or formula lone pairs are pairs of dots that are placed around an atomic symbol but are NOT between 2 atomic symbols. O H Lewis dot formula for oxygen Note: It doesn t matter on which side the lone electrons or the electron pairs in the Lewis dot formula are placed. So, the Lewis dot formula above is just of 4 possible arrangements.
3 Unit 3 Ray Tedder s Chemistry I Test Prep Guide page 3 Oxygen (symbol O) has only has 6 valence electrons. These electrons are represented by the 2 arrows above 2s and the 4 arrows above 2p in the orbital notation. These electrons are also represented by the superscript 2 in 2s 2 and the superscript 4 in 2p 4 in the orbital notation. It is also represented by the 6 dots around the hydrogen symbol in the Lewis dot formula. Recall that you put one dot on each of the 4 sides of the imaginary square around the oxygen symbol and then pair up dots if necessary until you reach the required number of dots. Now then, let s put these 2 Lewis dot formulas next to each other and see how we can share electrons to give hydrogen the 2 electrons (or dots) that it needs to have a full valence level and give oxygen the 8 electrons (or dots) that it needs to have a full valence level. You should write this down with me as I draw it. H Let s be clear about a couple of terms. A lone pair is a pair of electrons drawn on the same side of the atomic symbol. Hydrogen does not have a lone pair. Oxygen has 2 lone pairs. Oxygen also has 2 lone or single electrons. Now, let s draw a circle around the lone electron on hydrogen and one of the lone electrons around oxygen. This is how we predict the covalent bonding of hydrogen and oxygen. Hydrogen now has 2 electrons and that s all that it wants. Oxygen on the other hand now has 7 electrons. The problem is that oxygen wants 8 electrons. To get another electron, we need another hydrogen atom, like this: See how the 2 nd hydrogen has shared its electron? Now, oxygen has 8 electrons. This drawing is now called the Sharing arrangement for this molecule, but it s not yet the Lewis dot structure for the molecule. Now sharing arrangement is not some special scientific term. It s just my description used so that you and I both know of what is being spoken. We re ready to write the Lewis dot structure. See figure 3.1. All we do is to squeeze the dots we drew circles around between the atomic symbols. O H H O O Figure 3.1. This is an illustration of the Lewis dot structure for water. The dots H O represent electrons. Between each of the 2 hydrogen atoms and the oxygen there are 2 shared electrons or dots (point to these H dots that are between the H and the O). In addition, there are dots that represent electrons that are not shared. These unshared pairs of electrons are also called lone pairs (point to these pairs of dots on the top and on the right side of O). Notice that this arrangement gives oxygen 8 electrons and the 2 hydrogen atom s 2 electrons. This arrangement stabilizes all of these atoms. OK, let s try another one. This time let s write the Lewis dot formulas for an atom of hydrogen and a Lewis dot formula for an atom on chlorine. First, here is the orbital notation, the electron configuration, and the electron dot notation for chlorine. H
4 Unit 3 Ray Tedder s Chemistry I Test Prep Guide page 4 Cl: 2s 2p 3s 3p Cl: 2 2s 2 2p 6 3s 2 3p 5 Cl Here is an illustration of how carbon and chlorine combine to make a combination of carbon and chlorine to make carbon tetrachloride (CCl 4 ): Orbital notation for chlorine Electron configuration for chlorine Lewis dot formula for chlorine So, the correct electron dot notation for hydrogen and chlorine is below. H Cl Now I will write the correct sharing arrangement and you can check your work. H Cl Now, let s write a Lewis dot formula for the covalent bonding of these 2 electron dot notations for these 2 atoms. Here is the correct Lewis dot formula for the covalent bonding of these 2 elements and you can check your work. H Cl Now, we complete this whole process for a combination of H N H nitrogen and oxygen. The H N H correct sharing arrangement and Lewis dot formula for the covalent bonding of these 2 H elements is seen below. H Cl Cl C Cl Cl Cl Cl C Cl Cl
5 Unit 3 Ray Tedder s Chemistry I Test Prep Guide page 5 Lewis structures, Lewis diagrams, Lewis formulas In Lewis structures the valence electrons that are lone pairs are represented as dots and lines are used to represent shared pairs in a single, double, or triple bond. Lewis structures show each atom and its position in the structure of the molecule using its chemical symbol. Lines are drawn between atoms that are bonded to one another. One line represents 2 electrons that are shared in a bond. Excess electrons that form lone pairs are represented as pairs of dots, and are placed next to the atoms. Students should be able to determine the number of valence electrons. In the previous unit, students also learned how to determine the number of valance electrons from the orbital configuration and the electron configuration of the element. Students should also know that for the representative elements ONLY the number of valence electrons can be determined from the Roman numeral at the top of each column in which the element appears in the periodic table. Single bonds: H O Figure 3.2. An illustration of the Lewis structure or Lewis formula for water (compare to figure 3.2). By definition a single bond is a pair of electrons shared between the nuclei of two atoms bonded together. In a Lewis dot formula, a single bond is represented by a pair of electron dots between the atomic symbols for the bonded atoms. In a Lewis formula, a single bond is represented by a single line between the atomic symbols for the bonded atoms. Double bonds: By definition a double bond is two pairs of electrons shared between the nuclei of two atoms bonded together. In a Lewis dot formula, a double bond is represented by two pairs of electron dots between the atomic symbols for the bonded atoms. In a Lewis formula, a double bond is represented by a two parallel lines between the atomic symbols for the bonded atoms. Triple bonds: By definition a double bond is three pairs of electrons shared between the nuclei of two atoms bonded together. In a Lewis dot formula, a triple bond is represented by three pairs of electron dots between the atomic symbols for the bonded atoms. In a Lewis formula, a triple bond is represented by a three parallel lines between the atomic symbols for the bonded atoms. H Lines represent 2 electrons that are shared between 2 atoms (in this case hydrogen and oxygen) and dots represent in shared electrons (in this case the unshared electrons are in pairs so that are also called lone pairs ).
6 Unit 3 Ray Tedder s Chemistry I Test Prep Guide page 6 o Understand that crystalline structure is the result of the ionic bonding of positive ions and negative ions, forming a neutral compound. o Understand that ionic bonding of positive ions and negative ions forms a neutral compound. The sum of the oxidation numbers (or charge numbers) in the formula of any neutral compound is zero Ions are positively or negatively charged, atomic or molecular-sized particles. Ionic crystals Ions or ionic particles arrange themselves in such a way that positive charges are as close to negative charges as possible. The result is a regular, repeating structure called a lattice. When large enough for us to see, these ionic lattices are known as ionic crystals. Even though ionic compounds are made of charged particles, the positive and negative charges equal out so that the overall charge is 0 or neutral. Understand that metallic atoms can form positive monatomic ions by losing electrons in order to achieve a stable outer energy level electron structure. Metal ions typically have a small number of electrons in their outer or valence energy level. Representative element metals most often lose all their valence electrons, leaving the energy level that was below the valence level as the new outer level. This level has full s and p sublevels. The resulting ion has an electron configuration that is more stable than the atom that previously existed. Creating charged particles, however, creates a new kind of instability due to the charges that are formed. A charged particle is unstable because that charge seeks to establish equilibrium through neutralization. This charge instability problem can be solved by combining opposite charges in a ratio that neutralizes the charges. Note: Creating a charged particle, one that has an unequal number of protons and electrons, is called ionization Figure 3.3. Illustration of a small section of a crystal lattice. Note that most crystal lattices are more complex than this. Figure 3.4. This illustration of a periodic table outline shows the location of metals, non-metals and metalloids. Metalloids are elements that sometime behave like metals and sometimes behave like non-metals. Recall that electrons have a negative charge. Each time that an electron is removed from an atom or molecular structure the atom or structure is left with a + charge. This is because an atom has a neutral charge from having an equal number of positively charged protons and negatively charged electrons. Removing 1 electron creates a + charge, removing 2 electrons creates 2+ charge, removing 3 creates a 3+ charge, and so on. Taking electrons from an atom creates a
7 Unit 3 Ray Tedder s Chemistry I Test Prep Guide page 7 monoatomic ion and taking electrons from a molecule creates a polyatomic ion. Positive ions are called cations. Likewise, each time that an electron is added to an atom or molecular structure the electron brings with it a charge to that atom or molecular structure. Adding electrons to an atom creates a monoatomic ion and adding more electrons than protons to what would otherwise be a molecule creates a polyatomic ion. Negative ions are called anions. In other words, a monoatomic ion is a single atom with too many or too few electrons to have a neutral charge. Examples include: Na +, Mg 2+, Al 3+, P 3. O 2, and Cl all of which can be found on your periodic table of oxidation numbers in your test references. A polyatomic ion is a covalently bonded group of atoms with too many or too few electrons to have a neutral charge. Examples include: IO 2, IO 3, NO 3, NO 2, BrO 4, ClO 4, IO 4, BrO 3, BrO 2, ClO 3, CO 2 3, PO 3 4, and PO 3 3 all of which are found in the Common ions chart in your test references. Positively charged ions are called cations. Examples include: Na +, Mg 2+, Al 3+, and NH + 4. Negatively charged ions are called anions. Examples include: IO 2, IO 3, NO 3, NO 2, BrO 4, ClO 4, IO 4, BrO 3, BrO 2, ClO 3, CO 2 3, PO 3 4, and PO 3 3 aio 2, IO 3, NO 3, NO 2, BrO 4, ClO 4, IO 4, BrO 3, BrO 2, ClO 3, CO 2 3, PO 3 4, PO 3 3, P 3, O 2, and Cl. Sometimes a metal will become more stable by simply loosing all of its valence p-sublevel electrons, leaving a full and more stable s sublevel in the valence level. These electrons don t just disappear. They go somewhere. When thinking about ionic bonding between metal and non-metal atoms, it s helpful to think about the electrons lost by the metal being gained by the non-metal. See the next item. o Understand that nonmetal atoms can form negative monatomic ions by gaining electrons in order to achieve a stable outer energy level electron structure. Non-metal ions typically have a large number of electrons in their outer or valence energy level. Non-metals often gain enough extra electrons to fill their valence level (a full valence level for most atoms has 8 electrons). This valence level, with the extra electrons needed to reach 8 in the valence level, will also have full s and p sublevels and full orbitals. All these create additional stability. The resulting ion, therefore, is more stable than the atom that previously existed. When you write the electron configuration of calcium after it has lost 2 electrons, you MUST include the 2+ charge as a superscript on the calcium symbol (Ca 2+ ). Likewise, when you write the electron configuration of sulfur after it has gained 2 electrons, you MUST include the 2 charge as a superscript on the sulfur symbol (S 2 ).
8 Unit 3 Ray Tedder s Chemistry I Test Prep Guide page 8 Example: Using orbital notation, here is a way to think about it. The electrons that calcium wants to give up go to sulfur like this: Ca: S: S 2 : 2s 2s 2p 2p 3s 3s 3p 3p Using Lewis dot notation, here is still another way to think about it. Once again the electrons that calcium wants to give up go to sulfur like this: And because electrons have a negative charge the result is: Note the brackets around the sulfide ion. Because the 2 charge is outside the brackets, it communicates to you and me that the charge is shared by the entire structure. Sometimes we don t write it that way (we write it S 2 ) and we expect the reader to understand that the charge is shared over the whole structure. In the case of calcium and sulfur, calcium and sulfur had just the right number of electrons for sulfur. In the case of some other sets of atoms (which become ions) you may need 2, 3, 4 or any other number of metal or non-metal ions to get everything worked out to the most stable form. In all the cases above, the resulting formula unit of calcium sulfide is CaS. Notice when we put the 2 ions together there are no charges. That s because the 2+ charge is canceled out by the 2 charge and the resulting calcium sulfide compound is neutral. 4s And because electrons have a negative charge the result is: Ca 2+ : 2s 2p 3s 3p 2s 2p. C. 3s 3p.. S.. :.. Ca 2+ 2 : S.. :
9 Unit 3 Ray Tedder s Chemistry I Test Prep Guide page 9 Unhybridzed p x orbital hybridizes into an hybrid orbital P y p z p x Unhybridzed p z orbital hybridizes into an hybrid orbital p x p z p y Unhybridzed s orbital hybridizes into an hybrid orbital Unhybridzed p y orbital hybridizes into an hybrid orbital Figure 3.5. Recall that s and p orbitals that are not hybridized have the arrangement in the illustration above left. In the valence electron energy level, when electrons with this arrangement of orbitals bond, the orbitals hybridize. If the result of bonding creates a total of 4 single bonds plus lone pairs (# of lone electron pairs) + (# of single bonds) = 4 hybridized orbitals then the kind of hybridization that is illustrated on the right occurs. This kind of hybridization is called. It is called because the 4 orbitals stem from one s orbital and three p orbitals. Figure 3.21 and figure 3.22 illustrate the 2 other kinds of hybridization that you need to understand in a high school chemistry class.
10 Unit 3 Ray Tedder s Chemistry I Test Prep Guide page 10 P y p z p x s p x p z p y The unhybridzed 3s orbital below corresponds to the spherical s orbital illustration above The unhybridzed 3p orbital below corresponds to any of the double balloon shaped p orbital illustrations above The hybridzed 3 orbitals below correspond to any of the single balloon shaped orbital illustrations above Cl: 2s 2p 3s 3p Cl: 2s 2p 3 Unhybridized orbital notation for chlorine Unhybridized orbital notation for chlorine Figure 3.6. Recall that orbital notation is a bookkeeping system and does not show the actual shape of orbitals. The illustrations above show the relationships between orbital notations and the actual shape of valence level orbitals. Valence electrons: Valence electrons are those electrons in the highest primary energy level of an atoms electron cloud. In the illustrations above, the valence electrons are in the 3 rd primary level of chlorine. Valence electrons include those in the s and p sublevels in that highest level, so chlorine has 7 valence electrons.
Often times we represent atoms and their electrons with Lewis Dot Structures.
They are trying to get their number of valence electrons to either 0 or 8. Group 1: 1 valence electron Group 2: 2 valence electrons Group 13: 3 valence electrons Group 14: 4 valence electrons Group 15:
More informationUnit 3 Ray Tedder s Chemistry I CP Text page 125
Unit 3 Ray Tedder s Chemistry I CP Text page 125 Your Key Chemistry Annotation Guide If you are NOT using the following annotation, put in your key to the left of each item. Mr. T s Key Items to be annotated
More informationChapter 8: Bonding. Section 8.1: Lewis Dot Symbols
Chapter 8: Bonding Section 8.1: Lewis Dot Symbols The Lewis electron dot symbol is named after Gilbert Lewis. In the Lewis dot symbol, the element symbol represents the nucleus and the inner electrons.
More informationChemical Bond An attraction between the nuclei and valence electrons of different atoms, which binds the atoms together
Chemical Bond An attraction between the nuclei and valence electrons of different atoms, which binds the atoms together When atoms form chemical bonds their valence electrons move around. This makes atoms
More informationChemical Bonds, Lewis Structures, Bond Order, and Formal Charge
Chemical Bonds, Lewis Structures, Bond Order, and Formal Charge PRELAB ASSIGNMENT Read the entire laboratory write up. Write an objective, any hazards associated with this lab, and answer the following
More informationChapter 8. Chemical Bonding: Basic Concepts
Chapter 8. Chemical Bonding: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely
More informationChapter 8. Chemical Bonding: Basic Concepts
Chapter 8. Chemical Bonding: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely
More informationUnit 5: Diversity of Matter
20 20 Table of Contents Unit 5: Diversity of Matter Chapter 20: Chemical Bonds 20.1: Stability in Bonding 20.2: Types of Bonds 20.3: Writing Formulas and Naming Compounds 20.1 Compounds Stability in Bonding
More informationChemical Bonds. Chapter 6
Chemical Bonds Chapter 6 1 Ch. 6 Chemical Bonding I. How and Why Atoms Bond A. Vocabulary B. Chemical Bonds - Basics C. Chemical Bonds Types D. Chemical Bonds Covalent E. Drawing Lewis Diagrams F. Bond
More informationIts Bonding Time. Chemical Bonds CH 12
Its Bonding Time Chemical Bonds CH 12 What is a chemical bond? Octet Rule: Chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its
More informationChapter 12. Chemical Bonding
Chapter 12 Chemical Bonding Chapter 12 Introduction to Chemical Bonding Chemical Bonding Valence electrons are the electrons in the outer shell (highest energy level) of an atom. A chemical bond is a mutual
More informationElements combine to form compounds chemical bonds. Chemical Bonding
Elements combine to form compounds chemical bonds Chemical Bonding Review Valence electrons Using periodic table to determine them. General bonding rules: If an atom has 1 to 3 valence electrons, it will
More informationChapter 6 Chemistry Review
Chapter 6 Chemistry Review Multiple Choice Identify the choice that best completes the statement or answers the question. Put the LETTER of the correct answer in the blank. 1. The electrons involved in
More informationCovalent Bonding. a. O b. Mg c. Ar d. C. a. K b. N c. Cl d. B
Covalent Bonding 1. Obtain the number of valence electrons for each of the following atoms from its group number and draw the correct Electron Dot Notation (a.k.a. Lewis Dot Structures). a. K b. N c. Cl
More informationCHEMICAL BONDING COVALENT BONDS IONIC BONDS METALLIC BONDS
CHEMICAL BONDING COVALENT BONDS IONIC BONDS METALLIC BONDS Metallic Bonds How atoms are held together in solid metals. Metals hold onto their valence electrons very weakly. Think of them as positive ions
More informationCHEM 121 Introduction to Fundamental Chemistry. Summer Quarter 2008 SCCC. Lecture 5.
CHEM 121 Introduction to Fundamental Chemistry Summer Quarter 2008 SCCC Lecture 5 http://seattlecentral.edu/faculty/lcwest/che121 Forces Between Particles Noble Gas Configurations Ionic Bonding Ionic Compounds
More informationUNIT 4: Bonding CHEMICAL BONDS
UNIT 4: Bonding CHEMICAL BONDS A. Definition: B. Bonds form from the attraction between 1., or 2.. C. REVIEW 1. What part of the atom is involved in bonding? 2. Atoms bond to. What makes an atom stable?!
More informationChapter 6 Chemical Bonding
Chapter 6 Chemical Bonding Section 6-1 Introduction to Chemical Bonding Chemical Bonds Valence electrons are attracted to other atoms, and that determines the kind of chemical bonding that occurs between
More informationIONIC BONDING NOTES (Chapter 7 Section 1)
IONIC BONDING NOTES (Chapter 7 Section 1) I. Introduction Because all atoms want to have a total of, atoms will,, or electrons to form bonds. One of these bonds is an. A. Ionic Bond - is when a charged
More informationChapter 8 The Concept of the Chemical Bond
Chapter 8 The Concept of the Chemical Bond Three basic types of bonds: Ionic - Electrostatic attraction between ions (NaCl) Metallic - Metal atoms bonded to each other Covalent - Sharing of electrons Ionic
More informationIonic Bonding Ionic bonding occurs when metals and nonmetals trade one or more electrons and the resulting opposite charges attract each other. Metals
Chemical Bonding Now that we know what atoms look like A very small (less than 0.001% of the volume) and massive (more than 99.99% of the mass) nucleus with protons (+) and neutrons (neutral) and electrons
More informationChemical Bonding. Section 1 Introduction to Chemical Bonding. Section 2 Covalent Bonding and Molecular Compounds
Chemical Bonding Table of Contents Section 1 Introduction to Chemical Bonding Section 2 Covalent Bonding and Molecular Compounds Section 3 Ionic Bonding and Ionic Compounds Section 4 Metallic Bonding Section
More informationLewis Structures. Lewis Structures. Lewis Structures. Lewis Structures. What pattern do you see? What pattern do you see?
Look at the following chart: IA IIA IIIA IVA VA VIA VIIA VIIIA 2s1 2s2 2s22p1 2s22p2 2s22p3 2s22p4 2s22p5 2s22p6 The Roman Numerals are the Group numbers from the Periodic Table, Beneath them is the outer
More informationCHEM 1305 Introductory Chemistry
CHEM 1305 Introductory Chemistry Introductory Chemistry: Concepts and Critical Thinking 7 th Edition, Charles H. Corwin Chapter 12. Chemical Bonding Modified by: Dr. Violeta F. Coarfa 1 Chemical Bond Concept
More informationChapter 11 Chemical Bonds: The Formation of Compounds from Atoms Advanced Chemistry Periodic Trends in Atomic Properties Learning Objective
Chapter 11 Chemical Bonds: The Formation of Compounds from Atoms Advanced Chemistry 11.1 Periodic Trends in Atomic Properties Discuss the atomic trends Metals are located on the left side of the periodic
More informationIB Chemistry. Chapter 4.1
IB Chemistry Chapter 4.1 Chemical Bonds Atoms or ions that are strongly attached to one another Chemical bonds will form if potential energy decreases (becomes more stable) 2 Valence Electrons Valence
More informationChapter 7 Chemical Bonding
Chapter 7 Chemical Bonding 7.1 Ionic Bonding Octet rule: In forming compounds atoms lose, gain or share electrons to attain a noble gas configuration with 8 electrons in their outer shell (s 2 p 6 ), except
More informationWhat is Bonding? The Octet Rule. Getting an Octet. Chemical Bonding and Molecular Shapes. (Chapter Three, Part Two)
Chemical Bonding and Molecular Shapes (Chapter Three, Part Two) What is Bonding? Bonding describes how atoms interact with each other in an attractive sense. There are three types of bonding: Ionic bonding
More informationAtoms have the ability to do two things in order to become isoelectronic with a Noble Gas.
CHEMICAL BONDING Atoms have the ability to do two things in order to become isoelectronic with a Noble Gas. 1.Electrons can be from one atom to another forming. Positive ions (cations) are formed when
More informationChapter 10. Valence Electrons. Lewis dot symbols. Chemical Bonding
Chapter 10 Chemical Bonding Valence Electrons Recall: the outer electrons in an atom are valence electrons. Valence electrons are related to stability Valence electrons can be represented with dots in
More informationNotes: Electrons and Periodic Table (text Ch. 4 & 5)
Name Per. Notes: Electrons and Periodic Table (text Ch. 4 & 5) NOTE: This set of class notes is not complete. We will be filling in information in class. If you are absent, it is your responsibility to
More informationCHEMICAL BONDING IONIC BONDS COVALENT BONDS HYDROGEN BONDS METALLIC BONDS
CHEMICAL BONDING IONIC BONDS COVALENT BONDS HYDROGEN BONDS METALLIC BONDS IONIC BONDING When an atom of a nonmetal takes one or more electrons from an atom of a metal so both atoms end up with eight valence
More informationBond formation between two Hydrogen Atoms
Name Chem 162, Section: Group Number: ALE 9. Covalent Bonding (Reference: Section 9.3 - Silberberg 5 h edition) What determines the length of a covalent bond? The Model: Interactions that determine the
More informationNoble gases do not join other atoms to form compounds. They seem to be most stable just as they are.
UNIT 3: TE NATURE MATTER: MLECULES There are fewer than one hundred naturally occurring elements on the earth, but there are billions of compounds made of those elements. In this unit, we will examine
More informationIGCSE Double Award Extended Coordinated Science
IGCSE Double Award Extended Coordinated Science Chemistry 3.4 - Ions and Ionic Bonds Ions You need to know what ions are and how they can be formed. An ion is a charged atom, or a molecule - Caused by
More informationUnit 7: Basic Concepts of Chemical Bonding. Chemical Bonds. Lewis Symbols. The Octet Rule. Transition Metal Ions. Ionic Bonding 11/17/15
Unit 7: Basic Concepts of Chemical Bonding Topics Covered Chemical bonds Ionic bonds Covalent bonds Bond polarity and electronegativity Lewis structures Exceptions to the octet rule Strength of covalent
More informationChapter 8: Concepts of Chemical Bonding
Chapter 8: Concepts of Chemical Bonding Learning Outcomes: Write Lewis symbols for atoms and ions. Define lattice energy and be able to arrange compounds in order of increasing lattice energy based on
More informationUNIT 7 DAY 1. Ionic Bonding Basics; Dot diagrams
UNIT 7 DAY 1 Ionic Bonding Basics; Dot diagrams U7D1: Ionic Bonding Basics HW: See Schedule; Lab Due Thursday Do Now: 1.Write your name, date and period on all packets. 2.Look through schedule 3. answer
More information15.2 Electrons and Chemical Bonds
CHAPTER 15: MOLECULES AND COMPOUNDS 15.2 Electrons and Chemical Bonds The discovery of energy levels in the atom solved a 2,000-year-old mystery. The mystery was why elements combined with other elements
More informationCh 6 Chemical Bonding
Ch 6 Chemical Bonding What you should learn in this section (objectives): Define chemical bond Explain why most atoms form chemical bonds Describe ionic and covalent bonding Explain why most chemical bonding
More informationHonors Chemistry Unit 6 ( )
Honors Chemistry Unit 6 (2017-2018) Lewis Dot Structures VSEPR Structures 1 We are learning to: 1. Represent compounds with Lewis structures. 2. Apply the VSEPR theory to determine the molecular geometry
More informationAlso see lattices on page 177 of text.
Chemistry Ch 6 sect 3 «F_Name» «L_Name» Period «Per» «num» 6-3-1 Compare and contrast a chemical formula for a molecular compound with one for an ionic compound. Bond: Attraction between 2 or more atoms
More informationGeneral Chemistry Notes Name
Bio Honors General Chemistry Notes Name Directions: Carefully read the following information. Look for the ** directions in italics** for prompts where you can do some work. Use the information you have
More informationChapter 6. Preview. Objectives. Molecular Compounds
Section 2 Covalent Bonding and Molecular Compounds Preview Objectives Molecular Compounds Formation of a Covalent Bond Characteristics of the Covalent Bond The Octet Rule Electron-Dot Notation Lewis Structures
More informationIntroduction to Chemical Bonding
Chemical Bonding Introduction to Chemical Bonding Chemical bond! is a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together Why are most
More informationElectronic Structure and Bonding Review
Name: Band: Date: Electronic Structure and Bonding Review 1. For electrons: a. What is the relative charge? b. What is the relative mass? c. What is the symbol? d. Where are they located in the modern
More informationChapter 4: Forces Between Particles
Chapter 4: Forces Between Particles NOBLE GAS CONFIGURATIONS An electronic configuration that is characterized by two electrons in the valence shell of helium and eight electrons in the valence shell of
More informationa) DIATOMIC ELEMENTS e.g. . MEMORIZE THEM!!
CH 11 TOPIC 20 MOLECULAR COMPOUNDS COVALENT BONDS 1 You have mastered this topic when you can: 1) define or describe MOLECULAR ELEMENTS and DIATOMIC ELEMENTS. 2) define or describe MOLECULAR COMPOUND and
More informationChemical Bonding. Chemical Bonds. Metals, Ions, or Molecules. All Matter Exists as Atoms,
Chemical Bonding Valence electrons (the outer most electrons) are responsible for the interaction between atoms when forming chemical compounds. Another way to say that is that valence electrons are the
More informationUnit 3 - Part 1: Bonding. Objective - to be able to understand and name the forces that create chemical bonds.
Unit 3 - Part 1: Bonding Objective - to be able to understand and name the forces that create chemical bonds. Bonding: Key Terms to Know 1. Chemical formula 2. Molecular formula 3. Bond Energy 4. Bond
More informationChemistry 101 Chapter 12 Chemical Bonding
Chemistry 101 Chapter 12 Chemical Bonding Octet rule-duet role: when undergoing chemical reaction, atoms of group 1A-7A elements tend to gain, lose, or share sufficient electrons to achieve an electron
More informationChapter 8. Ions and the Noble Gas. Chapter Electron transfer leads to the formation of ionic compounds
Chapter 8 Chemical Bonding: General Concepts 1 8.1 Electron transfer leads to the formation of ionic compounds Ionic compounds form when metals and nonmetals react The attraction between positive and negative
More informationGilbert Kirss Foster. Chapter 4. Chemical Bonding. Understanding Climate Change
Gilbert Kirss Foster Chapter 4 Chemical Bonding Understanding Climate Change Chapter Outline 4.1 Types of Chemical Bonds 4.2 Naming Compounds and Writing Formulas 4.3 Lewis Structures 4.4 Electronegativity,
More informationBalancing Chemical Equations By Brian Goldstein
Balancing Chemical Equations By Brian Goldstein Help... Click Click Click to see the previous page to see the next page to return to the Table of Contents Table Of Contents The Atom Electrons Reactivity
More informationIntroduction to Chemical Bonding Chemical Bond
Introduction to Chemical Bonding Chemical Bond Mutual attraction between the and electrons of different atoms that binds the atoms together. Ionic Bond o that results from the attraction between large
More informationChapter 6. Preview. Lesson Starter Objectives Chemical Bond
Preview Lesson Starter Objectives Chemical Bond Section 1 Introduction to Chemical Bonding Lesson Starter Imagine getting onto a crowded elevator. As people squeeze into the confined space, they come in
More informationCHEM 101 Introduction to Fundamental Chemistry. Spring Quarter 2008 SCCC. Lecture 17.
CHEM 101 Introduction to Fundamental Chemistry Spring Quarter 2008 SCCC Lecture 17 http://seattlecentral.edu/faculty/lcwest/che101 Forces Between Particles Noble Gas Configurations Ionic Bonding Ionic
More informationCh 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules
Fructose Water Ch 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules Carbon Dioxide Ammonia Title and Highlight TN Ch 10.1 Topic: EQ: Right Side NOTES
More informationFocus Learning Targets for Periodic Trends and Bonding (1) Discuss the development of the periodic table by Mendeleev. (2) Locate and state important
Focus Learning Targets for Periodic Trends and Bonding (1) Discuss the development of the periodic table by Mendeleev. (2) Locate and state important properties of main chemical families including the
More informationDo Now. What are valence electrons?
Do Now What are valence electrons? Bonding Think of an atom as a HOTEL the front desk is the nucleus. Each room can hold a maximum of 2 electron guests, or a total of 8 electrons per floor. Except the
More informationChapter 12. Chemical Bonding
Chapter 12 Chemical Bonding Chemical Bond Concept Recall that an atom has core and valence electrons. Core electrons are found close to the nucleus. Valence electrons are found in the most distant s and
More informationCovalent Bonding H 2. Using Lewis-dot models, show how H2O molecules are covalently bonded in the box below.
Covalent Bonding COVALENT BONDS occur when atoms electrons. When atoms combine through the sharing of electrons, are formed. What is a common example of a covalently bonded molecule? When hydrogen atoms
More informationCh. 12 Section 1: Introduction to Chemical Bonding
Name Period Date Chemical Bonding & Intermolecular Forces (Chapter 12, 13 &14) Fill-in the blanks during the PowerPoint presentation in class. Ch. 12 Section 1: Introduction to Chemical Bonding Chemical
More informationChapter 6: Ionic and Molecular Compounds
Chapter 6: Ionic and Molecular Compounds 1. Recall that the group number indicates the number of valence electrons for any element in that group. Each noble gas has eight valence electrons (except helium,
More informationName Honors Chemistry / /
Name Honors Chemistry / / Lewis Structures & Resonance Structures Last chapter we studied ionic compounds. In ionic compounds electrons are gained or lost. In this chapter we are going to study covalent
More informationCHEMISTRY Matter and Change Section 8.1 The Covalent Bond
CHEMISTRY Matter and Change Section Chapter 8: Covalent Bonding CHAPTER 8 Table Of Contents Section 8.2 Section 8.3 Section 8.4 Section 8.5 Naming Molecules Molecular Structures Molecular Shapes Electronegativity
More informationChapter 7: Chemical Bonding and Molecular Structure
Chapter 7: Chemical Bonding and Molecular Structure Ionic Bond Covalent Bond Electronegativity and Bond Polarity Lewis Structures Orbital Overlap Hybrid Orbitals The Shapes of Molecules (VSEPR Model) Molecular
More informationC H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 7 CHEMICAL BONDING & MOLECULAR STRUCTURE INSTR : FİLİZ ALSHANABLEH
C H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 7 CHEMICAL BONDING & MOLECULAR STRUCTURE 0 1 INSTR : FİLİZ ALSHANABLEH CHAPTER 7 CHEMICAL BONDING & MOLECULAR STRUCTURE The Ionic Bond Formation of Ions The
More informationChemical Bonds CH. 18: PG
Chemical Bonds CH. 18: PG. 552-571 Today s Learning Objectives How does a compound differ from the elements that make it up? What is a chemical bond? Know how to determine the number of valence electrons
More informationLewis Dot diagrams. Developing and using models to predict formulas for stable, binary ionic compounds based on balance of charges
Lewis Dot diagrams 1. Developing and using models to predict formulas for stable, binary ionic compounds based on balance of charges 1 Lewis Dot Diagrams Refresher Element symbol is the centerpiece, surrounded
More informationChapter 6. Preview. Lesson Starter Objectives Chemical Bond
Preview Lesson Starter Objectives Chemical Bond Section 1 Introduction to Chemical Bonding Lesson Starter Imagine getting onto a crowded elevator. As people squeeze into the confined space, they come in
More informationChapter 6. Chemical Bonding
Chapter 6 Chemical Bonding Section 6.1 Intro to Chemical Bonding 6.1 Objectives Define chemical bond. Explain why most atoms form chemical bonds. Describe ionic and covalent bonding. Explain why most chemical
More informationCHAPTER 12 CHEMICAL BONDING
CHAPTER 12 CHEMICAL BONDING Core electrons are found close to the nucleus, whereas valence electrons are found in the most distant s and p energy subshells. The valence electrons are responsible for holding
More informationWhat does the word BOND mean to you?
Chemical Bonds What does the word BOND mean to you? Chemical Bond attractive force between atoms or ions in a molecule or compound. Formed by: transferring e - (losing or gaining) sharing e - What do you
More informationBonding. Honors Chemistry 412 Chapter 6
Bonding Honors Chemistry 412 Chapter 6 Chemical Bond Mutual attraction between the nuclei and valence electrons of different atoms that binds them together. Types of Bonds Ionic Bonds Force of attraction
More informationChapter 9 Bonding. Dr. Sapna Gupta
Chapter 9 Bonding Dr. Sapna Gupta Lewis Dot Symbol Lewis dot symbols is a notation where valence electrons are shown as dots. Draw the electrons symmetrically around the sides (top, bottom, left and right)
More informationIonic Bonding and Ionic Compounds
Main Ideas Ionic bonds form from attractions between positive and negative ions Differences in attraction strength give ionic and molecular compounds different properties Multiple atoms can bond covalently
More informationChapter 12 Structures and Characteristics of Bonds Objectives
Objectives 1. To learn about ionic and covalent bonds and explain how they are formed - what holds compounds together? 2. To learn about the polar covalent bond are all covalent bonds equal? 3. To understand
More informationWhat is a Bond? Chapter 8. Ionic Bonding. Coulomb's Law. What about covalent compounds?
Chapter 8 What is a Bond? A force that holds atoms together. Why? We will look at it in terms of energy. Bond energy- the energy required to break a bond. Why are compounds formed? Because it gives the
More informationINTRODUCTORY CHEMISTRY Concepts and Critical Thinking
INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Sixth Edition by Charles H. Corwin Chapter 12 Chemical Bonding by Christopher Hamaker 2011 Pearson Education, Inc. Chapter 12 1 Chemical Bond Concept
More informationCHAPTER 12: CHEMICAL BONDING
CHAPTER 12: CHEMICAL BONDING Problems: 1-26, 27c, 28, 33-34, 35b, 36(a-c), 37(a,b,d), 38a, 39-40, 41-42(a,c), 43-58, 67-74 12.1 THE CHEMICAL BOND CONCEPT chemical bond: what holds atoms or ions together
More informationChapter 7. Ionic & Covalent Bonds
Chapter 7 Ionic & Covalent Bonds Ionic Compounds Covalent Compounds 7.1 EN difference and bond character >1.7 = ionic 0.4 1.7 = polar covalent 1.7 Electrons not shared at
More informationIonic Bonding (Ch.7) Covalent Bonding (Ch.8) Metallic Bonding
Unit 3: Chemical Bonding Outline Ionic Bonding (Ch.7) Valence electrons Positive and negative ions and transition metal ions Ionic bonding: Charge on compounds Ionic compounds characteristics Writing ionic
More informationUnit 7. Bonds and Naming
Unit 7 Bonds and Naming I. Ionic Bonds Positive ion is attracted to a negative ion; usually a metal & a nonmetal Ionic compound: a substance that has ionic bonds Cation: positive ion Anion: negative ion
More informationAtoms with a complete outer shell do not react with other atoms. The outer shell is called the valence shell. Its electrons are valence electrons.
Bonding and the Outer Shell Use this table for reference: http://www.dreamwv.com/primer/page/s_pertab.html Atoms with incomplete shells react with others in a way that allows it to complete the outer shell.
More informationTest Review # 5. Chemistry: Form TR5-8A. Average Atomic Mass. Subatomic particles.
Chemistry: Form TR5-8A REVIEW Name Date Period Test Review # 5 Subatomic particles. Type of Particle Location Mass Relative Mass Charge Proton Center 1.67 10-27 kg 1 +1 Electron Outside 9.11 10-31 kg 0-1
More informationChapter 7. Chemical Bonding I: Basic Concepts
Chapter 7. Chemical Bonding I: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely
More informationBonding and structure: Forces Between Particles
Bonding and structure: Forces Between Particles NOBLE GAS CONFIGURATIONS An electronic configuration that is characterized by two electrons in the valence shell of helium and eight electrons in the valence
More informationBonding in Chemistry. Chemical Bonds All chemical reactions involve breaking of some bonds and formation of new ones where new products are formed.
CHEMICAL BONDS Atoms or ions are held together in molecules or compounds by chemical bonds. The type and number of electrons in the outer electronic shells of atoms or ions are instrumental in how atoms
More informationElectron Configuration in Ionic Bonding Ionic Bonds Bonding in Metals
Electron Configuration in Ionic Bonding Ionic Bonds Bonding in Metals Valence Electrons Electrons in the highest occupied energy level of an element s atoms Examples Mg: 1s 2 2s 2 2p 6 3s 2 2 valence e
More informationWold of Chemistry Notes for Students [Chapter 12, page 1] Chapter 12 Chemical Bonding
Wold of Chemistry Notes for Students [Chapter 12, page 1] Chapter 12 Chemical Bonding 1) The History of the Development of the Period Table (Not in the book!) Similarities between the chemical and physical
More informationThe Arrangement of Atoms in the Periodic Table
1 The Arrangement of Atoms in the Periodic Table [Material is from The Free High School Science Texts: Textbooks for High School Students Studying the Sciences Chemistry Grades 10 12. www.fhsst.org unless
More informationName: Hr: 8 Basic Concepts of Chemical Bonding
8.1-8.2 8.3-8.5 8.5-8.7 8.8 Name: Hr: 8 Basic Concepts of Chemical Bonding 8.1 Chemical Bonds, Lewis Symbols, and the Octet Rule State the type of bond (ionic, covalent, or metallic) formed between any
More informationLewis Structures (The Localized Electron Model)
Lewis Structures (The Localized Electron Model) G. N. Lewis 1875-1946 Using electron-dot symbols, G. N. Lewis developed the Localized Electron Model of chemical bonding (1916) in which valence electrons
More informationLewis Structures. .. : Br : Localized Electron Model. Lewis structures are representations of molecules showing all electrons, bonding and nonbonding.
Lewis Structures (The Localized Electron Model) G. N. Lewis 1875-1946 Localized Electron Model Using electron-dot symbols, G. N. Lewis developed the Localized Electron Model of chemical bonding (1916)
More informationELECTRONS. Construct your own electron dot diagram Choose one element & drag the correct number of VALENCE Br electrons around it.
Ch. 6 - Chemical Bonds Chemical reactivity depends on electron configuration. Remember the Stable Octet rule: when the highest energy level occupied is filled with electrons (8 electrons for most atoms),
More informationFormation of Ions. Ions formed when atoms gain or lose valence e - to achieve a stable octet
Ionic Bonding Formation of Ions Ions formed when atoms gain or lose valence e - to achieve a stable octet Cation Positively charged ion Forms when atom loses electrons Anion negatively charged ion Forms
More informationCovalent Bonding. Click a hyperlink or folder tab to view the corresponding slides. Exit
Covalent Bonding Section 8.1 The Covalent Bond Section 8.2 Naming Molecules Section 8.3 Molecular Structures Section 8.4 Molecular Shapes Section 8.5 Electronegativity and Polarity Click a hyperlink or
More informationUnit Five Practice Test (Part I) PT C U5 P1
Unit Five Practice Test (Part I) PT C U5 P1 Name Period LPS Standard(s): --- State Standard(s): 12.3.1 Short Answers. Answer the following questions. (5 points each) 1. Write the electron configuration
More information6.1 Intro to Chemical Bonding Name:
6.1 Intro to Chemical Bonding Name: A. Chemical bond Favored by nature because: 3 main types of bonds 1. 2. 3. B. Ionic Bonds C. Covalent Bonds D. Metallic Bond E. Bond Determination RECALL: Electronegativity
More information